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Questions and Answers
Which of the following salts is guaranteed to be soluble in water?
Which of the following salts is guaranteed to be soluble in water?
What will be the potential precipitate when mixing solutions of cesium bromide and lead (II) nitrate?
What will be the potential precipitate when mixing solutions of cesium bromide and lead (II) nitrate?
Which of the following compounds falls under the category of sparingly soluble substances?
Which of the following compounds falls under the category of sparingly soluble substances?
Which of the following is a notable exception to the solubility of sulfates in water?
Which of the following is a notable exception to the solubility of sulfates in water?
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When predicting solubility, which of the following ions does NOT indicate a compound that is soluble?
When predicting solubility, which of the following ions does NOT indicate a compound that is soluble?
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Which of the following statements about sparingly soluble hydroxides is incorrect?
Which of the following statements about sparingly soluble hydroxides is incorrect?
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In a double-displacement reaction between Na2CO3 and BaCl2, what would be the likely result?
In a double-displacement reaction between Na2CO3 and BaCl2, what would be the likely result?
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Which combination of substances will definitely produce a precipitate when mixed?
Which combination of substances will definitely produce a precipitate when mixed?
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What characterizes ionic compounds in solution under most conditions?
What characterizes ionic compounds in solution under most conditions?
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Why do ionic compounds like KCl dissolve in water?
Why do ionic compounds like KCl dissolve in water?
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Which of the following is an example of an insoluble compound?
Which of the following is an example of an insoluble compound?
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In a double-replacement reaction between sodium nitrate and ammonium chloride, what is the expected outcome?
In a double-replacement reaction between sodium nitrate and ammonium chloride, what is the expected outcome?
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What role do solubility rules play in predicting precipitates?
What role do solubility rules play in predicting precipitates?
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What happens to the disorder of a system when ionic compounds dissolve?
What happens to the disorder of a system when ionic compounds dissolve?
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Which factor can prevent an ionic compound from dissolving in water?
Which factor can prevent an ionic compound from dissolving in water?
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What is a spectator ion?
What is a spectator ion?
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Which of the following compounds is classified as soluble?
Which of the following compounds is classified as soluble?
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What type of reaction occurs when a soluble compound and an insoluble product form?
What type of reaction occurs when a soluble compound and an insoluble product form?
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Which compound is classified as an electrolyte?
Which compound is classified as an electrolyte?
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What is the net ionic equation for a precipitation reaction involving Pb2+ and Br-?
What is the net ionic equation for a precipitation reaction involving Pb2+ and Br-?
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Which of the following statements about solubility rules is true?
Which of the following statements about solubility rules is true?
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Which of the following ions is considered a spectator ion in a reaction involving cesium nitrate?
Which of the following ions is considered a spectator ion in a reaction involving cesium nitrate?
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Which compound is known to be insoluble due to the presence of lead(II) ions?
Which compound is known to be insoluble due to the presence of lead(II) ions?
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Which of the following compounds is classified as a nonelectrolyte?
Which of the following compounds is classified as a nonelectrolyte?
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Study Notes
Chemical Reactions
- Chemical reactions are processes that transform one or more substances into one or more new substances.
- Substances initially present are reactants, with new substances formed as products. Atoms are neither created nor destroyed.
- Chemical reactions are confirmed by observable changes, such as color change, energy exchange (heat or light), gas production, precipitate formation, and property change.
Evidence of a Chemical Reaction
- A chemical change always produces matter differing from the initial form.
- Examples include: rust forming, combustion, cooking, digestion, and decomposition.
The Chemical Equation
- Reactants and products are identified using chemical formulas.
- Reactants are written before the arrow "→", which separates them from the products written to the right.
- Subscripts in formulas indicate the ratio of atoms in a molecule.
- Coefficients in front of formulas indicate the number of molecules in a reaction.
How to Write Balanced Chemical Equations
- Coefficients, not subscripts, are adjusted to balance equations.
- The law of conservation of mass dictates that the number and type of atoms on both sides of a balanced equation must be equal.
- A balanced chemical equation displays a precise ratio of reactants and products involved in the reaction.
- Simple steps to balance an equation include: identifying the most complex molecule, adjusting coefficients for the elements in only that molecule, and finishing with adjusting coefficients for the remaining elements.
Aqueous Solutions and Solubility- Compounds Dissolved in Water
- Electrolytes are substances that dissolve in water to produce ions, with strong electrolytes dissolving completely, and weak electrolytes partially.
- Nonelectrolytes do not produce ions when dissolved in water.
- Conductivity is measured by the dissolved ions' concentration, the electrical current through electrodes in the solution, influencing the bulb's brightness.
- Ions and polar molecules, like water, are attracted by ion-dipole interactions, facilitating dissolution.
Precipitation Reactions
- When two solutions containing soluble ionic compounds mix, an insoluble product (precipitate) can form, often with color change.
- Predicting reactions (or lack thereof) can be determined by examining possible products and their solubility rules.
Writing Chemical Equations in Solution
- Molecular equations represent the overall reaction, including the states of reactants and products (solid, liquid, gas, aqueous).
- Complete ionic equations show all ions present in the solution.
- Spectator ions, ions that do not participate, are omitted in the net ionic equation, focusing on the reacting species.
Acid-Base and Gas Evolution Reactions
- Reactions between acids and bases (neutralization reactions) produce water and salt (ionic compound).
- Gas evolution reactions involve the production of a gaseous product, often when acids react with carbonates or bicarbonates.
- Examples include reactions creating CO2, H2S, or other gases.
Oxidation-Reduction Reactions
- Oxidation involves a loss of electrons or a gain of oxygen; reduction involves a gain of electrons or a loss of oxygen.
- Redox reactions involve the transfer of electrons from one reactant to another.
- Oxidation numbers are used to track electrons during redox reactions.
Classifying Chemical Reactions
- Chemical reactions generally fit into five types including acid-base, combination (synthesis), decomposition, single replacement, and double replacement.
The Activity Series- Predicting Spontaneous Redox Reactions
- The activity series ranks elements based on their tendency to lose or gain electrons in redox reactions, predicting spontaneous single displacement reactions (metal replacement).
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